Chemical Equilibrium Factors

What is Le Chatelier's Principle?

• Le Chatelier's Principle is used to predict the future of a system at equilibrium.

• Le Chatelier's Principle only applies to chemical reactions involving gases.

• Le Chatelier's Principle states that equilibrium is always reached in a closed system.

• Le Chatelier's Principle describes how systems at equilibrium respond to external changes.

How does temperature affect chemical equilibrium?

• Temperature decreases the concentration of reactants at equilibrium

• Temperature has no effect on chemical equilibrium

• Temperature affects chemical equilibrium by changing the equilibrium constant.

• Temperature increases the rate of reaction at equilibrium

Explain the effect of pressure on equilibrium.

• Pressure affects equilibrium by shifting it towards the side with fewer gas molecules to reduce the pressure.

• Pressure has no effect on equilibrium

• Pressure increases the rate of reaction at equilibrium

• Pressure causes equilibrium to shift towards the side with more gas molecules

Discuss the influence of concentration on equilibrium.

• Le Chatelier's Principle explains that if the concentration of reactants or products is increased, the equilibrium will shift to consume the added substance and establish a new equilibrium position.

• Equilibrium is only influenced by temperature, not concentration.

• Concentration has no impact on equilibrium.

• Increasing concentration leads to a decrease in the equilibrium constant.

What role does a catalyst play in chemical equilibrium?

• Speeds up the attainment of equilibrium by lowering activation energy

• Delays the attainment of equilibrium by increasing activation energy

• Causes a shift in equilibrium towards the reactants

• Has no effect on the attainment of equilibrium

How do changes in volume impact equilibrium?

• Changes in volume have no impact on equilibrium

• Changes in volume always shift equilibrium to the left

• Changes in volume only impact equilibrium for solid-phase reactions

• Changes in volume can shift the equilibrium position of a reaction to favor the side with fewer moles of gas when the volume decreases and to favor the side with more moles of gas when the volume increases.

Describe the effect of adding or removing a reactant on equilibrium.

• Adding a reactant has no effect on equilibrium

• Removing a reactant shifts equilibrium towards products

• Adding a reactant shifts equilibrium towards products; removing a reactant shifts equilibrium towards reactants.

• Adding a reactant shifts equilibrium towards reactants

What is the significance of equilibrium constant in chemical reactions?

• Equilibrium constant remains constant throughout the reaction

• The significance of equilibrium constant in chemical reactions lies in its ability to quantify the balance between products and reactants at equilibrium.

• Equilibrium constant determines the rate of a chemical reaction

• Equilibrium constant is only relevant for exothermic reactions

Explain the concept of dynamic equilibrium.

• Dynamic equilibrium involves a constant increase in reactants and decrease in products.

• Dynamic equilibrium occurs only in irreversible reactions.

• Dynamic equilibrium is achieved in a reversible reaction when the rates of the forward and reverse reactions are equal, leading to a constant concentration of reactants and products.

• Dynamic equilibrium is achieved when the reaction stops completely.

Discuss the effect of changing the reaction conditions on equilibrium.

• Adjusting reaction conditions only affects the rate of reaction, not the equilibrium position

• Altering reaction conditions always shifts the equilibrium to the left

• Changing reaction conditions has no impact on equilibrium

• Changing reaction conditions can affect the equilibrium position by favoring either the forward or reverse reaction, ultimately leading to a new equilibrium state.